US20130095362A1 - Vanadium flow cell - Google Patents

Vanadium flow cell Download PDF

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Publication number
US20130095362A1
US20130095362A1 US13/651,230 US201213651230A US2013095362A1 US 20130095362 A1 US20130095362 A1 US 20130095362A1 US 201213651230 A US201213651230 A US 201213651230A US 2013095362 A1 US2013095362 A1 US 2013095362A1
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solution
electrolyte
hcl
cell
acid
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Abandoned
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US13/651,230
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English (en)
Inventor
Majid Keshavarz
Ge Zu
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IMERGY POWER SYSTEMS Inc
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Deeya Energy Inc
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Priority to KR1020147012836A priority Critical patent/KR20140083027A/ko
Priority to CN201280060862.2A priority patent/CN103975463A/zh
Priority to US13/651,230 priority patent/US20130095362A1/en
Priority to AU2012323979A priority patent/AU2012323979A1/en
Priority to JP2014535961A priority patent/JP2014532284A/ja
Priority to PCT/US2012/060129 priority patent/WO2013056175A1/en
Priority to IN2817CHN2014 priority patent/IN2014CN02817A/en
Priority to BR112014009075A priority patent/BR112014009075A2/pt
Application filed by Deeya Energy Inc filed Critical Deeya Energy Inc
Publication of US20130095362A1 publication Critical patent/US20130095362A1/en
Assigned to DEEYA ENERGY, INC. reassignment DEEYA ENERGY, INC. ASSIGNMENT OF ASSIGNORS INTEREST (SEE DOCUMENT FOR DETAILS). Assignors: KESHAVARZ, MAJID, ZU, GE
Priority to ZA2014/02826A priority patent/ZA201402826B/en
Assigned to IMERGY POWER SYSTEMS, INC. reassignment IMERGY POWER SYSTEMS, INC. CHANGE OF NAME (SEE DOCUMENT FOR DETAILS). Assignors: DEEYA ENERGY, INC.
Priority to US14/526,435 priority patent/US20150050570A1/en
Abandoned legal-status Critical Current

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    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M8/00—Fuel cells; Manufacture thereof
    • H01M8/18—Regenerative fuel cells, e.g. redox flow batteries or secondary fuel cells
    • H01M8/184—Regeneration by electrochemical means
    • H01M8/188—Regeneration by electrochemical means by recharging of redox couples containing fluids; Redox flow type batteries
    • H—ELECTRICITY
    • H01—ELECTRIC ELEMENTS
    • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
    • H01M8/00—Fuel cells; Manufacture thereof
    • H01M8/20—Indirect fuel cells, e.g. fuel cells with redox couple being irreversible
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
    • Y02E60/30—Hydrogen technology
    • Y02E60/50—Fuel cells

Definitions

  • Embodiments disclosed herein generally relate to Vanadium based flow cell batteries.
  • a redox flow cell battery may include one or more redox flow cells.
  • Each of the redox flow cells may include positive and negative electrodes disposed in separate half-cell compartments. The two half-cells may be separated by a porous or ion-selective membrane, through which ions are transferred during a redox reaction. Electrolytes (anolyte and catholyte) are flowed through the half-cells as the redox reaction occurs, often with an external pumping system. In this manner, the membrane in a redox flow cell battery operates in an aqueous electrolyte environment.
  • Redox flow cell battery performance may change based on parameters such as the state of charge, temperature, electrolyte level, concentration of electrolyte and fault conditions such as leaks, pump problems, and power supply failure for powering electronics.
  • Vanadium based flow cell system have been proposed for some time.
  • challenges in developing a Vanadium based system include, for example, the high cost of the Vanadium electrolyte, the high cost of appropriate membranes, the low energy density of dilute electrolyte, thermal management, impurity levels in the Vanadium, inconsistent performance, stack leakage, membrane performance such as fouling, electrode performance such as delamination and oxidation, rebalance cell technologies, and system monitoring and operation.
  • Embodiments of the present invention provide a vanadium based flow cell system.
  • a method for providing an electrolytic solution according to the present invention includes chemically reducing an acidic solution/suspension of V5+ to form a reduced solution and electrochemically reducing the reduced solution to form an electrolyte.
  • a flow cell battery system includes a positive vanadium electrolyte; a negative vanadium electrolyte; and a stack having a plurality of cells, each cell formed between two electrodes and having a positive cell receiving the positive vanadium electrolyte and a negative cell receiving the negative vanadium electrolyte separated by a porous membrane.
  • FIG. 1 shows a vanadium based redox flow cell according to some embodiments of the present invention in a system.
  • FIG. 2 illustrates a method of providing a vanadium electrolyte.
  • FIG. 3A illustrates production of a balanced electrolyte according to some embodiments of the present invention.
  • FIG. 3B illustrates production of electrolytes according to some embodiments of the present invention.
  • FIG. 1 illustrates a vanadium based flow system 100 according to some embodiments of the present invention.
  • system 100 is coupled between power sources 102 and a load 104 .
  • Power sources 102 can represent any source of power, including an AC power grid, renewable power generators (solar, wind, hydro, etc.), fuel generators, or any other source of power.
  • Load 104 can represent any user of power, for example a power grid, building, or any other load devices.
  • redox flow cell system 100 includes redox flow cell stack 126 .
  • Flow cell stack 126 illustrates a single cell, which includes two half-cells 108 and 110 separated by a membrane 116 , but in most embodiments is a collection of multiple individual cells.
  • An electrolyte 128 is flowed through half-cell 108 and an electrolyte 130 is flowed through half-cell 110 .
  • Half-cells 108 and 110 include electrodes 120 and 118 , respectively, in contact with electrolytes 128 and 130 , respectively, such that redox reactions occur at the surface of the electrodes 120 or 118 .
  • multiple redox flow cells 126 may be electrically coupled (e.g., stacked) either in series to achieve higher voltage or in parallel in order to achieve higher current.
  • the stacked cells 126 are collectively referred to as a battery stack and flow cell battery can refer to a single cell or battery stack.
  • electrodes 120 and 118 are coupled across power converter 106 , through which electrolytes 128 and 130 are either charged or discharged.
  • half-cell 110 of redox flow cell 100 When filled with electrolyte, half-cell 110 of redox flow cell 100 contains anolyte 130 and the other half-cell 108 contains catholyte 128 , the anolyte and catholyte being collectively referred to as electrolytes.
  • Reactant electrolytes may be stored in separate reservoirs 124 and 122 , respectively, and dispensed into half-cells 108 and 110 via conduits coupled to cell inlet/outlet (I/O) ports.
  • I/O cell inlet/outlet
  • an external pumping system is used to transport the electrolytes to and from the redox flow cell.
  • At least one electrode 120 and 118 in each half-cell 108 and 110 provides a surface on which the redox reaction takes place and from which charge is transferred.
  • Redox flow cell system 100 operates by changing the oxidation state of its constituents during charging or discharging.
  • the two half-cells 108 and 110 are connected in series by the conductive electrolytes, one for anodic reaction and the other for cathodic reaction. In operation (e.g., during charge or discharge), electrolytes 126 and 124 are flowed through half-cells 108 and 110 .
  • Electrolyte is flowed through half-cell 108 from holding tank 124 , the positive electrolyte, by a pump 112 . Electrolyte is flowed through half-cell 110 from holding tank 122 , the negative electrolyte, through pump 114 .
  • Holding tank 124 during operation, holds an electrolyte formed from V 5+ and V 4+ species while holding tank 122 holds an electrolyte formed from V 2 and V 3+ species.
  • a balanced electrolyte a 1:1 ratio of V3+ and V4+
  • an initial charging results in the V 3 ⁇ in tank 122 being converted to V 4+ and the V 4+ in tank 122 being converted to V 3+ .
  • membrane 116 Separats the two half-cells 108 and 110 , as the redox flow cell 100 charges or discharges.
  • Reactant electrolytes are flowed through half-cells 108 and 110 , as necessary, in a controlled manner to supply electrical power or be charged through power converter 106 .
  • Suitable membrane materials for membrane 106 include, but are not limited to, materials that absorb moisture and expand when placed in an aqueous environment.
  • membrane 106 may comprise sheets of woven or non-woven plastic with active ion exchange materials such as resins or functionalities embedded either in a heterogeneous (such as co-extrusion) or homogeneous (such as radiation grafting) way.
  • membrane 106 may be a porous membrane having high voltaic efficiency Ev and high coulombic efficiency and may be designed to limit mass transfer through the membrane to a minimum while still facilitating ionic transfer.
  • membrane 106 may be made from a polyolefin material or fluorinated polymers and may have a specified thickness and pore diameter.
  • a manufacturer having the capability to manufacture these membranes, and other membranes consistent with embodiments disclosed, is Daramic Microporous Products, L.P., N. Community House Rd., Suite 35, Charlotte, N.C. 28277.
  • membrane 106 may be a nonselective microporous plastic separator also manufactured by Daramic Microporous Products L.P.
  • a flow cell formed from such a membrane is disclosed in U.S. Published Patent App. No. 2010/0003586, filed on Jul. 1, 2008, which is incorporated herein by reference.
  • membrane 116 can be any material that forms a barrier between fluids, for example between electrochemical half-cells 108 and 110 (e.g., an anode compartment and a cathode compartment).
  • Exemplary membranes may be selectively permeable, and may include ion-selective membranes.
  • Exemplary membranes may include one or more layers, wherein each layer exhibits a selective permeability for certain species (e.g., ions), and/or effects the passage of certain species.
  • the open circuit voltage of each cell in stack 126 is then 1.25V, ( ⁇ 0.25 V from half-cell 110 and 1.00V from half-cell 108 ).
  • ions H + and Cl ⁇ (or sulfate) may traverse membrane 116 during the reaction.
  • multiple redox flow cells may be stacked to form a redox flow cell battery system.
  • Construction of a flow cell stack battery system is described in U.S. patent application Ser. No. 12/577,134, entitled “Common Module Stack Component Design” filed on Oct. 9, 2009, which is incorporated herein by reference.
  • Embodiments of the invention disclosed herein attempt to solve many of the challenges involved with utilizing a Vanadium chemistry in a redox flow cell. As such, this disclosure is separated into three sections: I. Preparation of the Electrolyte; II. Formulation of the Electrolyte; and III. The flow cell battery system.
  • Vanadium electrolyte can be very expensive to prepare. In previous efforts, VOSO 4 is utilized as a starting material for preparation of the electrolyte. However, VOSO 4 is very expensive to procure and VOCl 2 is not commercially available.
  • the correct oxidation state of vanadium, as starting material, for vanadium redox flow battery is V 4+ for positive side and V 3+ for negative side or a 1:1 mixture of V 4+ and V 3+ for both sides, which is often referred to as V 3.5+ or “balanced electrolyte.”
  • the electrolyte material can be formed from a V 5+ compound such as V 2 O 5 . V 2 O 5 is much less expensive to procure than is VOSO 4 , and is much more readily available. The electrolyte is then formed of lower oxidation states of the V 5+ of V 2 O 5 .
  • a vanadium electrolyte is formed from a source of V 5+ by adding a reducing agent and an acid.
  • a method of producing a vanadium based electrolyte is illustrated in procedure 200 shown in FIG. 2 .
  • step 202 includes creating a solution and/or suspension of Vanadium and acid.
  • the solution or suspension includes V 5+ .
  • V 5+ can be obtained, for example, with the compounds V 2 O 5 , MVO 3 , or M 3 VO 4 , where M can be NH 4+ , Na + , K + , or some other cations, although some of these compounds may leave impurities and undesired ions in the electrolyte.
  • the acid can be H 2 SO 4 , HCl, H 3 PO 4 , CH 3 SO 3 H, or a mixture of these acids.
  • the acid is a mixture of H 2 SO 4 and HCl.
  • only HCl is utilized.
  • H 2 SO 4 has been utilized as the acid in the electrolyte.
  • a combination of HCl and H 2 SO 4 or all HCl can be utilized in some embodiments.
  • step 204 a reducing agent is added to the Vanadium containing acid solution formed in step 202 .
  • the general reaction is given by
  • the reducing agent can be an organic reducing agent or an inorganic reducing agent.
  • Organic reducing agents include one carbon reagents, two carbon reagents, three carbon reagents, and four or higher carbon reagents.
  • One carbon reducing agents include methanol, formaldehyde, formic acid, and nitrogen containing functional groups like acetamide or sulfur containing functional groups like methyl mercaptane or phosphorous functional groups.
  • methanol formaldehyde, formic acid, and nitrogen containing functional groups like acetamide or sulfur containing functional groups like methyl mercaptane or phosphorous functional groups.
  • one such reaction starts with methanol as follows:
  • reaction methanol to formaldehyde to formic acid provides the reduction of the V 5+ , resulting in the emission of CO 2 .
  • the electrons go to reducing the vanadium charge state.
  • the reaction can also begin with formaldehyde or formic acid or any mixture of them.
  • Two carbon reducing agents include ethanol, acetaldehyde, acetic acid, ethylene glycol, glycol aldehyde, oxaldehyde, glycolic acid, glyoxalic acid, oxalic acid, nitrogen containing functional groups such as 2-aminoethanol, sulfur containing functional groups like ethylene dithiol.
  • One such reaction starts with ethylene glycol and ends again with CO2:
  • Ethylene glycol C 2 H 4 (OH) 2 is very useful as a reducing agent since it provide 10 electrons and final product is gaseous carbon dioxide.
  • reducing agents include 1-propanol, 2-proponal, 1,2-propanediol, 1,3-propanedial, glycerol, propanal, acetone, propionic acid and any combination of hydroxyl, carbonyl, carboxylic acid, nitrogen containing functional groups, sulfur containing functional groups, and phosphourous functional groups.
  • glycerol is a great source of electrons that work like ethylene glycol. The only by-product is gaseous carbon dioxide and glycerol provides 14 electrons to the reduction reaction.
  • the chemical reduction utilizing glycerol can be described as:
  • carbon organic molecules with any combination of hydroxyl, carbonyl, carboxylic acid, nitrogen containing functional groups, sulfur containing functional groups, or phosphorous functional groups can be utilized.
  • sugar e.g. glucose or other sugar
  • sugar can be utilized.
  • Many of these reducing agents e.g., methanol glycerol, sugar, ethylene glycol
  • inorganic reducing agents can include, for example, sulfur, and sulfur dioxide. Any sulfide, sulfite, or thiosulfate salt can also be utilized. Sulfur compounds work great, especially if sulfate salt is desired in the final formulation. However, the resulting solution may have higher concentrations of sulfuric acid at completion of the process. Sulfide salts can be utilized, resulting in the added ions appearing in the solution at the end of the process. Additionally, vanadium metal can be utilized. Vanadium metal can easily give up four electrons to form V 4 ⁇ .
  • Secondary reducing agents which can be added in small quantities, can include any phosphorous acid, hypophophorous acid, oxalic acid and their related salts. Any nitrogen based reducing agent can be utilized. Further, metals can be included, for example Alkali metals, alkaline earth metals, and some transition metals like Zn and Fe.
  • step 204 of FIG. 2 can be assisted with heating or may proceed at room temperature. Reagent is added until the vanadium ion concentration is reduced as far as desired.
  • step 206 the acidity of the resulting vanadium electrolyte can be adjusted by the addition of water or of additional acid.
  • FIG. 3A illustrates a procedure 300 of producing vanadium based electrolyte according to some embodiments of the present invention.
  • a starting preparation of V 5+ e.g., an acidic solution/suspension of V 2 O 5
  • a chemical reducing reaction such as that illustrated in procedure 200 discussed above is performed to provide an acidic solution 304 of V 4+ , which is prepared from the reduction of V 2 O 5 as discussed above.
  • solution 304 may contain any reduction of V 5+ , e.g. V (5 ⁇ n)+ , however for purposes of explanation solution 304 can be an acidic solution of primarily V 4+ .
  • Solution 304 is then utilized to fill the holding tanks of an electrochemical cell.
  • the electrochemical cell can be, for example, similar to flow cell system 100 illustrated in FIG. 1 .
  • procedure 300 can utilize a flow cell 100 as illustrated in FIG. 1 that includes a single electrochemical cell.
  • a stack 126 that includes individual multiple cells can be utilized in procedure 300 .
  • the electrochemical cell can be a photochemical cell such as the rebalance cell described in U.S. patent application Ser. No. 12/790,753 entitled “Flow Cell Rebalancing”, filed May 28, 2010, which is incorporated herein by reference.
  • a cell can be utilized to generate low-valence vanadium species from V 5+ .
  • the rebalance cell is a redox reaction cell with two electrodes on either end and a membrane between the two electrodes that provides a negative side and a positive side.
  • the positive side includes an optical source that assists generating the HCl solution.
  • can be reduced to V 2 or the reduction can be stopped at V 4
  • HCl will be oxidized electrochemically to Cl 2 gas or, with the addition of H 2 , recombined in the photochemical chamber to regenerate HCl.
  • step 306 the electrochemical cell containing solution 304 is charged. Electrochemical charging can proceed to a nominal state of charge. This results in solution 308 , for example in tank 124 of flow cell 100 , containing V 5+ and solution 310 , for example in tank 122 of flow cell 100 , containing V 3+ .
  • the reaction may be stopped when solution 310 achieves a balanced electrolyte of 1:1 ratio of V 3+ and V 4+ (e.g., a SOC of 50%).
  • solution 310 can then be used as a balanced electrolyte in both the positive and negative sides of a flow cell battery such as flow cell 100 illustrated in FIG. 1 . As illustrated in FIG.
  • electrochemical charging 306 results in a solution 308 from the positive side of the electrochemical cell that includes V 5+ and a solution 310 from the negative side of the electrochemical cell that includes V 3+ .
  • Solution 308 can undergo further chemical reduction in process 200 and then be included in solution 304 .
  • FIG. 3B illustrates a procedure 320 for producing electrolyte according to some embodiments of the present invention.
  • Procedure 320 is similar to procedure 300 illustrated in FIG. 3A . However, in procedure 320 , electrochemical charging reaction 306 is allowed to proceed to a higher state of charge, in some cases close to 100%. In that case, solution 310 can be utilized as the negative electrolyte and solution 304 utilized as the positive electrolyte in a flow cell battery.
  • solution 302 can be formed utilizing any combination of acids.
  • solution 302 can be formed of HCl and be sulfur free (i.e. not include H2SO4), can be a mixture of HCl and H 2 SO 4 , or can be formed of H 2 SO 4 .
  • the resulting electrolyte can, in some cases, be sulfur free.
  • all chloride (sulfate free) electrolyte has been prepared with 2.5 Molar VO 2+ in 4 N HCl.
  • the total acid molarity can be from 1 to 9 molar, for example 1-6 molar.
  • the vanadium concentration can be between 0.5 and 3.5 M VO2+, for example 1.5 M, 2.5 M, or 3M VOCl 2 .
  • Higher concentration of vanadium have been prepared (e.g., 3.0 M vanadium in HCl) and utilized in a flow cell such as cell 100 .
  • Mixed electrolyte have also been prepared in HCl and sulfuric acid and utilized in a flow cell such as cell 100 .
  • All chloride (no sulfate or sulfate free electrolyte) is the most soluble and stable electrolytes at higher and lower temperatures, as sulfate anion reduces the solubility of vanadium species.
  • All chloride solutions can be heated up 65 C can be kept at 65 C for a long time, where as sulfate based solutions precipitate at 40 C.
  • Different ratios of sulfate and chloride can be prepared.
  • the total acid molarity can be from 1 to 9 molar, for example 1-3 molar.
  • the vanadium concentration can be between 1 and 3.5 M VOSO 4 .
  • a catalyst can also be added to the electrolyte.
  • 5 ppm of Bi 3+ for example Bismuth chloride or bismuth oxide can be added. This concentration can range from 1 ppm to 100 ppm.
  • Other catalysts that can be utilized include lead, indium, tin, antimony, and thallium.
  • solution 304 In one example preparation of solution 304 , a 400 L polyethylene reaction vessel equipped with a Teflon-coated mechanical stirrer and a Teflon-coated thermocouple was charged with DI water (22 L), glycerol (5.0 L) and 12 M HCl (229 L). V 2 O 5 (75.0 kg) was added in six installments over 2.5 hours while the heterogeneous mixture was self-heated to 60-70° C. The progress of the reaction was monitored by absorption spectroscopy (Ultraviolet-Visible) at different time intervals. After four hours of stirring the blue solution was filtered through five and one micron filters respectively. The concentration of V 4+ was measured by UV-VIS spectroscopy to be 3.0 M and the acid concentration was measured by titration to be 4 M. The volume of the solution was 275 L.
  • the flow cell system 100 is generally described in the applications incorporated by reference herein. Although those systems are described in the context of a Fe/Cr chemistry, the flow cell system 100 operates equally well with the vanadium chemistry described herein.
  • Tanks 122 and 124 can each be 200 liter tanks and the electrolyte formed from 1.15 M VOSO 4 /4.0 M HCl.
  • Stack 126 includes 22 individual cells with a general reaction area of 2250 cm 2 . Stack 126 can utilize Nippon 3 mm high density felt, Daramic membranes, Graphite foil bipolar plates, Ti current collectors. There is no rebalance cell and no plating procedure. A 150 A or higher charge can be utilized.

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IN2817CHN2014 IN2014CN02817A (zh) 2011-10-14 2012-10-12
US13/651,230 US20130095362A1 (en) 2011-10-14 2012-10-12 Vanadium flow cell
AU2012323979A AU2012323979A1 (en) 2011-10-14 2012-10-12 Vanadium flow cell
JP2014535961A JP2014532284A (ja) 2011-10-14 2012-10-12 バナジウムフローセル
PCT/US2012/060129 WO2013056175A1 (en) 2011-10-14 2012-10-12 Vanadium flow cell
KR1020147012836A KR20140083027A (ko) 2011-10-14 2012-10-12 바나듐 플로우 셀
BR112014009075A BR112014009075A2 (pt) 2011-10-14 2012-10-12 método para fornecer uma solução de eletrólito, e, sistema de bateria de célula de fluxo
CN201280060862.2A CN103975463A (zh) 2011-10-14 2012-10-12 钒液流电池
ZA2014/02826A ZA201402826B (en) 2011-10-14 2014-04-16 Vanadium flow cell
US14/526,435 US20150050570A1 (en) 2011-10-14 2014-10-28 Production of vanadium electrolyte for a vanadium flow cell

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US8916281B2 (en) 2011-03-29 2014-12-23 Enervault Corporation Rebalancing electrolytes in redox flow battery systems
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CN105990593A (zh) * 2015-01-30 2016-10-05 中国科学院过程工程研究所 一种高纯钒电池电解液的制备系统及方法
CN106299437A (zh) * 2016-11-11 2017-01-04 攀钢集团攀枝花钢铁研究院有限公司 钒电池及其负极电解液以及提高其电化学活性的方法
CN106463755A (zh) * 2014-06-13 2017-02-22 株式会社Lg化学 钒溶液、包含该钒溶液的电解液、包含该电解液的二次电池以及制备该钒溶液的方法
KR101736539B1 (ko) * 2014-06-02 2017-05-16 주식회사 엘지화학 플로우 배터리에 적용 가능한 전해액 농도 조절 모듈 및 이를 이용한 플로우 배터리의 전해액 농도 균형 조절 방법
WO2018047079A1 (en) * 2016-09-06 2018-03-15 Redt Ltd (Dublin, Ireland) Balancing of electrolytes in redox flow batteries
US20180108931A1 (en) * 2016-10-19 2018-04-19 Wattjoule Corporation Vanadium redox flow batteries
US10153502B2 (en) 2014-12-08 2018-12-11 Lockheed Martin Energy, Llc Electrochemical systems incorporating in situ spectroscopic determination of state of charge and methods directed to the same
US10186726B2 (en) 2013-10-16 2019-01-22 Lockheed Martin Energy, Llc Method and apparatus for measuring transient state-of-charge using inlet/outlet potentials
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